1. Metallic Bonding
Strong forces of attraction are responsible
for the high melting point of most metals.

2. CA Standards
Students know atoms combine to form
molecules by sharing electrons to form
covalent or metallic bonds or by
exchanging electrons to form ionic
bonds.

3. Metallic Bonding
 The chemical bonding that
results from the attraction
between metal cations and the
surrounding sea of electrons
 Vacant p and d orbitals in
metal's outer energy levels
overlap, and allow outer
electrons to move freely
throughout the metal
 Valence electrons do not
belong to any one atom

4. Packing in Metals
Model: Packing
uniform, hard
spheres to best use
available space.
This is called closest
packing. Each atom
has 12 nearest
neighbors.

5. Metal Alloys
Substitutional
Alloy: some metal
atoms replaced by
others of similar
size.

6. Metal Alloys
Interstitial Alloy:
Interstices (holes)
in closest packed
metal structure are
occupied by small
atoms.

7. Properties of Metals
 Metals are good
conductors of heat and
electricity
 Metals are malleable
 Metals are ductile
 Metals have high
tensile strength
 Metals have luster